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With respect to periodic properties, the CORRECT statement is

  • A.Electron affinity order is F \(\gt\) O \(\gt\) Cl
  • B.First ionisation energy order is Al \(\gt\) Mg \(\gt\) K
  • C.Atomic radius order is N \(\gt\) P \(\gt\) As
  • D.Ionic radius order is \(\text{K}^{+} \gt \text{Ca}^{2+} \gt \text{Mg}^{2+}\)

Answer: D

The correct statement is Ionic radius order is K+ > Ca2+ > Mg2+.

K+ and Ca2+ are isoelectronic (18 electrons); Ca2+ has one more proton, so it pulls the same electrons in more tightly and is smaller. Mg2+ has one shell fewer and is smaller still.

The other statements are wrong. Electron affinity runs Cl > F > O: fluorine's small, crowded 2p shell makes its electron affinity lower than chlorine's. First ionisation energy runs Mg > Al > K, because Al loses an easily removed 3p electron while Mg must lose one from a filled 3s subshell. Atomic radius increases down the group, so As > P > N.

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